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(A) The van der Waals equation for $1 \ mol$ of a gas is given by $(p + \frac{a}{V_m^2})(V_m - b) = RT$.At high temperature,the kinetic energy of gas

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$pV_m = RT$

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(A) The van der Waals equation for $1 \ mol$ of a gas is given by $(p + \frac{a}{V_m^2})(V_m - b) = RT$.At high temperature,the kinetic energy of gas molecules is very high,making the effect of intermolecular forces $(a/V_m^2)$ negligible.At low pressure,the volume of the gas $(V_m)$ is very large,making the excluded volume $(b)$ negligible compared to $V_m$.Under these conditions,the equation reduces to $pV_m = RT$,which is the ideal gas equation.

Gas	$a / (kPa \cdot dm^6 \cdot mol^{-2})$	$b / (dm^3 \cdot mol^{-1})$
$A$	$642.32$	$0.05196$
$B$	$155.21$	$0.04136$
$C$	$431.91$	$0.05196$
$D$	$155.21$	$0.4382$

What will the van der Waals equation be at high temperature and low pressure?

Similar Questions

Consider the following table:

Gas $a / (kPa \cdot dm^6 \cdot mol^{-2})$ $b / (dm^3 \cdot mol^{-1})$

$A$ $642.32$ $0.05196$

$B$ $155.21$ $0.04136$

$C$ $431.91$ $0.05196$

$D$ $155.21$ $0.4382$

$a$ and $b$ are van der Waals constants. The correct statement about the gases is:

The van der Waals equation of state for a real gas is given. For $n$ moles of a real gas,the equation can be expressed as:

Which of the following represents the $Van \ der \ Waals$ equation for $n$ moles of a real gas?

Explain real gases showing deviations from ideal gas with correction of pressure and volume and derive van der Waals equation.

Among the gases $a$,$b$,$c$,$d$,$e$ and $f$,the gases that show only positive deviation from ideal behavior at all pressures in the graph are

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